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In order to neutralize the acid in 10.0 mL of 18.0 mol/L sulfuric acid that was spilled on a laboratory bench, sodium bicarbonate (baking soda) was used. The container of baking soda had a mass of 155.00g before this use, and out of curiosity it's mass was measured as 144.50g afterward.

Write a balanced equation for the reaction between sulfuric acid and sodium bicarbonate.

was sufficient sodium bicarbonate used? identify by calculation the limiting and excess reactants.

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  1. H2SO4 + 2NaHCO3 ==> Na2SO4 + 2H2O + 2CO2

    mass NaHCO3 = 155.00-144.50 = 10.50 g used.

    mols NaHCO3 = grams/molar mass = about 0.125
    If all were to be used it would produce how many mols H2O. That is 0.125 mols NaHCO3 x (2 mols H2O/2 mols NaHCO3) = 0.125 mols CO2.

    mols H2SO4 = M x L = 18.0 x 0.010 = 0.18 mols.
    If all were to be used it would produce how many mols H2O? That's
    0.010 mols H2SO4 x (2 mols H2O/1 mol H2SO4) = 0.010 x 2/1 = 0.020

    In limiting reagent problems, the SMALLER number is the correct value; therefore, 0.02 mols CO2 will be produced, the H2SO4 is the limiting reagent, and NaHCO3 is the excess reagent. Therefore, all of the H2SO4 will be neutralized and NaHCO3 will be left over unreacted.

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